At their normal boiling points, the heat of vaporization of water (100^∘ C) is 40,656 J / mol a

step 1 The vapor pressure above a liquids increases non -linear as the temperature increases. So we can

At their normal boiling points, the heat of vaporization of...

At their normal boiling points, the heat of vaporization of water $\left(100^{\circ} \mathrm{C}\right)$ is $40,656 \mathrm{~J} / \mathrm{mol}$ and that of heavy water $\left(101.41^{\circ} \mathrm{C}\right)$ is $41,606 \mathrm{~J} / \mathrm{mol}$. Use these data to calculate the vapor pressure of each liquid at $80.00^{\circ} \mathrm{C}$.

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Key Concepts

Heat of Vaporization

Heat of vaporization, also known as the enthalpy of vaporization, is the amount of energy required to convert a given quantity of a liquid into vapor at constant temperature and pressure. This quantity directly influences the slope in the Clausius-Clapeyron equation and is essential for calculating changes in vapor pressure with temperature.

Temperature Conversion to Kelvin

In thermodynamic calculations, it is important to use the Kelvin scale because absolute temperature is required to ensure that formulas such as the Clausius-Clapeyron equation yield correct results. This conversion from Celsius to Kelvin is a fundamental step when working with these equations.

Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases (solid or liquid) at a given temperature. It is a critical concept in understanding phase transitions because it determines the point at which a liquid begins to boil and how its pressure changes with temperature.

Clausius-Clapeyron Equation

The Clausius-Clapeyron equation provides a way to relate the vapor pressure and temperature of a substance to its enthalpy of vaporization. This equation is integral in thermodynamics for predicting how the vapor pressure of a substance changes with temperature, especially between two known states.

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